![]() INHALATION: Remove the victim to fresh air. Large amounts of water should be used to rinse or flood the area of contact as small amounts of water may do more harm than good. General information: It is advisable to have tongs, tweezers, scrapers or some kind of implement on hand to remove bits of metal from skin or clothing in the event of an accident. Store in a closed container, P405 Store locked up, P501 Dispose of contents/container in accordance with local, state or federal regulations. Continue rinsing, P310 Immediately call a POISON CENTER or doctor/physician, P363 Wash contaminated clothing before reuse, P370+P378 In case of fire: Use class D metal extinguishing agent for extinction, do not use water, P402+P404 Store in a dry place. Remove contact lenses, if present and easy to do. Rinse SKIN with water/shower, P335+P334 Brush off loose particles from skin and immerse in cool water/wrap in wet bandages, P304+P340 IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing, P305+P351+P338 IF IN EYES: rinse cautiously with water for several minutes. Do NOT induce vomiting, P303+P361+P353 IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Protect from moisture, P260 Do not breath dust or fume, P264 Wash skin thoroughly after handling, P280 Wear protective gloves/protective clothing/eye protection/face protection, P301+P330+P331 IF SWALLOWED: rinse mouth. Precautionary Statements: P223 Keep away from any possible contact with water, because of violent reaction and possible flash fire, P231+P232 Handle under inert gas. Hazard Statements: H260 In contact with water releases flammable gases which may ignite spontaneously, H314 Causes severe skin burns and eye damage. GHS Classification (.1200): Substances and mixtures which, in contact with water, emit flammable gases, category 1, Skin corrosion/irritation, category 1B, Eye damage/irritation, category 1. You need JavaScript enabled to view it.Įmergency: Infotrac 80 (US) or 35 (24 hour) So we can add/subtract in chemical equations, but its can't just simply make mathematical sense, it also has to make sense in a chemistry context.Email: This email address is being protected from spambots. So it's not much that we're adding chemicals rather we're discovering the actual reaction occurring. However if it's an aqueous solution, these added chemicals are technically always present in the reaction solution and what we're actually doing is recognizing that some of them are actually part of the redox reaction. Now in this case where we're adding chemicals to the equation it may just seem like we're adding chemicals out of convenience to make the math work out. In redox reaction it's common to add water, H+, and OH- ion to the equations when balancing them. So since they're not participating in the reaction, subtract them is allowed because it doesn't affect the reaction if they're absent from the equation. So these are ions which are present in the reaction solution, but don't really participate in the actual reaction (they don't change as a product compared to when they were a reactant). For ionic equations like these it's possible for us to eliminate, essentially subtract out, spectator ions from an equation. Mathematically it's completely acceptable to do so, however we have to consider the actual chemical makeup of our reaction if we do so. In sodium chloride, the ion-dipole bonds release more energy than was required to break the ionic bonds so it is soluble, but for silver chloride the ion-dipole bonds release less energy than is required to break the ionic bonds so it is insoluble. If more energy is required to break the bonds than is released during bond formation, then the solid is insoluble. For the dissolution process to be successful, we must release more energy than is required to break the bonds. The same is true here.įor an ionic solid to dissolve, the solvent (in this case water) has to break the ionic bonds then surround the ions and form new ion-dipole bonds in a solvation shell. An energy input is required to break bonds, and energy is subsequently released when bonds are formed. The key is the energy associated with the dissolving process. While both are sodium chloride and silver chloride are ionic compounds, sodium chloride is soluble and dissolves easily in water while silver chloride is insoluble and does not dissolve much into water.
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